Stable electrolyte material and solvent material containing same

ABSTRACT

A chemical compound having the following chemical structure: 
     
       
         
           
             
               ⌊ 
               
                 
                   H 
                   x 
                 
                 ⁢ 
                 
                   O 
                   
                     
                       ( 
                       
                         x 
                         - 
                         1 
                       
                       ) 
                     
                     2 
                   
                 
               
               ⌋ 
             
             ⁢ 
             
               Z 
               y 
             
           
         
       
         
         
           
             wherein x is an odd integer ≥3; 
             y is an integer between 1 and 20; and 
             Z is one of a monoatomic ion from Groups 14 through 17 having a charge value between −1 and −3 or a polyatomic ion having a charge between −1 and −3.

CROSS-REFERENCE TO RELATED APPLICATION

This application claims priority to U.S. Provisional Patent ApplicationNo. 62/152,009, filed Apr. 23, 2015.

BACKGROUND

The present invention relates to compositions of matter that can beincorporated into various aqueous solutions rendering the resultingsolution either acidic or basic depending on the initial solutioncomposition.

It has been long accepted scientific fact that, based upon laws ofthermodynamics, the internal energy of a closed system is stable whenthe two different charge-types, i.e. moles of positively charged cations(+) and moles of negatively charged anions (−), are stoichiometricallycharge-balanced; yielding a stable charge neutral aqueous solution. Ithas been widely held that electrostatic charge types in a neutralsolution will necessarily have positive electrostatic charges (+)balanced by an equal number of negative (−) electrostatic charges.However, studies conducted on aqueous acidic solutions indicate thatvarious solutions may process an excess of acid proton ions.

This phenomenon supports the conclusion that water molecules areeffective in stabilizing unbalanced charges present in solution. It isbelieved that water molecules present in an aqueous solution stabilizeany unbalanced charges and yield a charge balanced solution. The resultsconform to the laws of thermodynamics and point to the presence of a newtype of charge balancing nucleophile composed of lone pair electrons ofwater molecules.

While the presence of unbalanced charges has been hypothesized, variousspecies of water molecules can exist in transient states. It is believedthat stable forms of complex water molecules would have desirablecharacteristics and properties if these could be identified andproduced. Thus, it would be desirable to produce a stable electrolytematerial that could be employed independently or used in a solutionmaterial.

SUMMARY

Disclosed herein is a composition of matter having the followingchemical structure:

$\lfloor {H_{x}O_{\frac{({x - 1})}{2}}} \rfloor Z_{y}$

-   -   wherein x is an odd integer ≥3;    -   y is an integer between 1 and 20; and    -   Z is a polyatomic ion or monoatomic ion.

Also disclosed is a solution that is composed of the compound

$\lbrack {{H_{x}O_{\frac{({x - 1})}{2}}} + ( {H_{2}O} )_{y}} \rbrack Z$

-   -   wherein x is an odd integer ≥3;    -   y is an integer between 1 and 20; and    -   Z is a polyatomic ion or monoatomic ion; wherein at least a        portion of the chemical composition is present as H₉O₄+ in        coordinated combination with H₉O₄+:SO₄H and working bridging        ligands containing stable hydronium (H₃O+) clusters.

DETAILED DESCRIPTION

Disclosed herein is a novel electrolyte that can be employed in aqueoussolutions that is broadly construed as an oxonium ion-derived complex.As defined herein “oxonium ion complexes” are generally defined aspositive oxygen cations having at least one trivalent oxygen bond. Incertain embodiments, the oxygen cation will exist in aqueous solution asa population predominantly composed of one, two and three trivalentlybonded oxygen cations present as a mixture of the aforesaid cations oras material having only one, two or three trivalently bonded oxygencations. Non-limiting examples of oxonium ions having trivalent oxygencations can include at least one of hydronium ions.

It is contemplated that the in certain embodiments the oxygen cationwill exist in aqueous solution as a population predominantly composed ofone, two and three trivalently bonded oxygen anions present as a mixtureof the aforesaid anions or as material having only one, two or threetrivalently bonded oxygen anions.

When the composition of matter as disclosed herein is admixed with asolvent such as an aqueous or organic solvent, the resulting compositionis a solution that can be composed of hydronium ions, hydronium ioncomplexes and mixtures of the same. Suitable cationic materials can alsobe referred to as hydroxonium ion complexes. The composition of matterand solutions that contain the same may have utility in variousapplications where low pH values are desirable. The compounds andmaterials disclosed herein may also have applicability in a variety ofsituations not limited to certain cleaning and sanitizing applications.

It has been theorized that extreme trace amounts of cationic hydroniummay spontaneously form in water from water molecules in the presence ofhydrogen ions. Without being bound to any theory, it is believed thatnaturally occurring hydronium ions are extremely rare. The concentrationof naturally occurring hydronium ions in water is estimated to be nomore than 1 in 480,000,000. If they occur at all, hydronium ioncompounds are extremely unstable. It is also theorized that naturallyoccurring hydronium ions are unstable transient species with lifespanstypically in the range of nanoseconds. Naturally occurring hydronium ionspecies are reactive and are readily solvated by water and as such thesehydronium ions (hydrons) do not exist in a free state.

When introduced into pure water, the stable hydronium material disclosedherein is one that will remain identifiable. It is believed that thestable hydronium material disclosed herein can complex with watermolecules to form hydration cages of various geometries, non-limitingexamples of which will be described in greater detail subsequently. Thestable electrolyte material as disclosed herein, when introduced into apolar solvent such as an aqueous solution is stable and can be isolatedfrom the associated solvent as desired or required.

Conventional strong organic and inorganic acids such as those having apK_(a)≥1.74, when added to water, will ionize completely in the aqueoussolution. The ions so generated will protonate existing water moleculesto form H₃O+ and associate stable clusters. Weaker acids, such as thosehaving a pK_(a)<1.74, when added to water, will achieve less thancomplete ionization in aqueous solution but can have utility in certainapplications. Thus, it is contemplated that the acid material employedto produce the stable electrolyte material can be a combination of oneor more acids. In certain embodiments, the acid material will include atleast one acid having a pK_(a) greater than or equal to 1.74 incombination with weaker acids(s).

In the present disclosure, it has been found quite unexpectedly that thestable hydronium electrolyte material as defined herein, when added toan aqueous solution, will produce a polar solvent and provide aneffective pK_(a) which is dependent on the amount of stable hydroniumelectrolyte material added to the corresponding solution independent ofthe hydrogen ion concentration originally present in that solution. Theresulting solution can function as a polar solvent and can have aneffective pK_(a) between 0 and 5 in certain applications when theinitial solution pH prior to addition of the stable hydronium materialis between 6 and 8.

It is also contemplated that the stable electrolyte material asdisclosed herein can be added to solutions having an initial pH in thealkaline range, for example between 8 and 12 to effectively adjust thepH of the resulting solvent and/or the effective or actual pK_(a) of theresulting solution. Addition of the stable electrolyte material asdisclosed herein can be added to an alkaline solution withoutperceivable reactive properties including, but not limited to,exothermicity, oxidation or the like.

The acidity of theoretical hydronium ions existing in water as a resultof aqueous auto-dissociation is the implicit standard used to judge thestrength of an acid in water. Strong acids are considered better protondonors than the theoretical hydronium ion material, otherwise asignificant portion of acid would exist in a non-ionized state. Asindicated previously, theoretical hydronium ions derived from aqueousauto-dissociation are unstable as a species, random in occurrence andbelieved to exist, if at all, in extreme low concentration in theassociated aqueous solution. Generally, hydronium ions in aqueoussolution are present in concentrations between less than 1 in480,000,000 and can be isolated, if at all, from native aqueous solutionvia solid or liquid phase organosynthesis as monomers attached to asuperacid solution in structures such as HF—SbF₅SO₂. Such materials canbe isolated only in extremely low concentration and decompose readilyupon isolation.

In contrast, the stable hydronium material as disclosed herein, providesa source of concentrated hydronium ions that are long lasting and can besubsequently isolated from solution if desired or required.

In certain embodiments, the composition of matter, has the followingchemical structure:

$\lbrack {{H_{x}O_{\frac{({x - 1})}{2}}} + ( {H_{2}O} )_{y}} \rbrack Z$

-   -   wherein x is an odd integer between 3-11;    -   y is an integer between 1 and 10; and    -   Z is a polyatomic or monoatomic ion.

The polyatomic ion Z can be an ion that is derived from an acid havingthe ability to donate one or more protons. The associated acid can beone that would have a pK_(a) values ≥1.7 at 23° C. The polyatomic ion Zemployed can be one having a charge of +2 or greater. Non-limitingexamples of such polyatomic ions include sulfate ions, carbonate ions,phosphate ions, oxalate ions, chromate ions, dichromate ions,pyrophosphate ions and mixtures thereof. In certain embodiments, it iscontemplated that the polyatomic ion can be derived from mixtures thatinclude polyatomic ions that include ions derived from acids havingpK_(a) values ≤1.7.

The stable electrolyte material as disclosed herein is stable atstandard temperature and pressure and can exist as an oily liquid. Thestable electrolyte material can be added to water or other polar solventto produce a polar solution that contains an effective concentration ofstable hydronium ion that is greater than 1 part per million. In certainembodiments, the stable electrolyte material as disclosed herein canprovide an effective concentration of stable hydronium ion material thatis greater than between 10 and 100 parts per million when admixed with asuitable aqueous or organic solvent.

It has been found, quite unexpectedly, that the hydronium ion complexespresent in solution as a result of the addition of the stableelectrolyte material disclosed herein alter the acid functionality ofthe resulting solvent material without a concomitant change in the freeacid to total acid ratio. The alteration in acid functionality caninclude characteristics such as change in measured pH, changes infree-to-total acid ratio, changes in specific gravity and rheology.Changes in spectral output and chromatography output are also noted ascompared to the incumbent acid materials used in production of thestable electrolyte material containing the initial hydronium ioncomplex. Addition of the stable electrolyte material as disclosed hereinresults in changes in pK_(a) which do not correlate to the changesobserved in free-to-total acid ratio.

Thus, the addition of the stable hydronium electrolyte material asdisclosed herein to an aqueous solution having an initial pH between 6and 8 results in a solution having an effective pK_(a) between 0 to 5.It is also to be understood that the pK_(a) of the resulting solutioncan exhibit a value less than zero as when measured by a calomelelectrode, specific ion ORP probe. As used herein the term “effectivepK_(a)” is a measure of the total available hydronium ion concentrationpresent in the resulting solvent. Thus, it is possible that pH and/orassociated pKa of a material when measured may have a numeric valuerepresented between −3 and 7.

Typically, the pH of a solution is a measure of its proton concentrationor as the inverse proportion of the —OH moiety. It is believed that thestable electrolyte material as disclosed herein, when introduced into apolar solution, facilitates at least partial coordination of hydrogenprotons with the hydronium ion electrolyte material and/or itsassociated lattice or cage. As such, the introduced stable hydronium ionelectrolyte material exists in a state that permits selectivefunctionality of the introduced hydrogen associated with the hydrogenion.

More specifically, the stable electrolyte material as disclosed hereincan have the general formula in certain embodiments:

$\lfloor {H_{x}O_{\frac{({x - 1})}{2}}} \rfloor Z_{y}$

-   -   x is an odd integer ≥3;    -   y is an integer between 1 and 20; and    -   Z is one of a monoatomic ion from Groups 14 through 17 having a        charge between −1 and −3 or a poly atomic ion having a charge        between −1 and −3.

In the composition of matter as disclosed herein, monatomic constituentsthat can be employed as Z include Group 17 halides such as fluoride,chloride, iodide and bromide; Group 15 materials such as nitrides andphosphides and Group 16 materials such as oxides and sulfides.Polyatomic constituents include carbonate, hydrogen carbonate, chromate,cyanide, nitride, nitrate, permanganate, phosphate, sulfate, sulfite,chlorite, perchlorate, hydrobromite, bromite, bromate, iodide, hydrogensulfate, hydrogen sulfite. It is contemplated that the composition ofmatter can be composed of a single one to the materials listed above orcan be a combination of one or more of the compounds listed.

It is also contemplated that, in certain embodiments, x is an integerbetween 3 and 9, with x being an integer between 3 and 6 in someembodiments.

In certain embodiments, y is an integer between 1 and 10; while in otherembodiments y is an integer between 1 and 5.

The composition of matter as disclosed herein can have the followingformula, in certain embodiments:

$\lfloor {H_{x}O_{\frac{({x - 1})}{2}}} \rfloor Z_{y}$

-   -   x is an odd integer between 3 and 12;    -   y is an integer between 1 and 20; and    -   Z is one of a group 14 through 17 monoatomic ion having a charge        between −1 and −3 or a poly atomic ion having a charge between        −1 and −3 as outlined above, some embodiments having x between 3        and 9 and y being an integer between 1 and 5.

It is contemplated that the composition of matter exists as an isomericdistribution in which the value x is an average distribution of integersgreater than 3 favoring integers between 3 and 10.

The composition of matter as disclosed herein can be formed by theaddition of a suitable inorganic hydroxide to a suitable inorganic acid.The inorganic acid may have a density between 22° and 70° baume; withspecific gravities between about 1.18 and 1.93. In certain embodiments,it is contemplated that the inorganic acid will have a density between50° and 67° baume; with specific gravities between 1.53 and 1.85. Theinorganic acid can be either a monoatomic acid or a polyatomic acid.

The inorganic acid employed can be homogenous or can be a mixture ofvarious acid compounds that fall within the defined parameters. It isalso contemplated that the acid may be a mixture that includes one ormore acid compounds that fall outside the contemplated parameters but incombination with other materials will provide an average acidcomposition value in the range specified. The inorganic acid or acidsemployed can be of any suitable grade or purity. In certain instances,tech grade and/or food grade material can be employed successfully invarious applications.

In preparing the stable electrolyte material as disclosed herein, theinorganic acid can be contained in any suitable reaction vessel inliquid form at any suitable volume. In various embodiments, it iscontemplated that the reaction vessel can be non-reactive beaker ofsuitable volume. The volume of acid employed can be as small as 50 ml.Larger volumes up to and including 5000 gallons or greater are alsoconsidered to be within the purview of this disclosure.

The inorganic acid can be maintained in the reaction vessel at asuitable temperature such as a temperature at or around ambient. It iswithin the purview of this disclosure to maintain the initial inorganicacid in a range between approximately 23° and about 70° C. However lowertemperatures in the range of 15° and about 40° C. can also be employed.

The inorganic acid is agitated by suitable means to impart mechanicalenergy in a range between approximately 0.5 HP and 3 HP with agitationlevels imparting mechanical energy between 1 and 2.5 HP being employedin certain applications of the process. Agitation can be imparted by avariety of suitable mechanical means including, but not limited to, DCservo drive, electric impeller, magnetic stirrer, chemical inductor andthe like.

Agitation can commence at an interval immediately prior to hydroxideaddition and can continue for an interval during at least a portion ofthe hydroxide introduction step.

In the process as disclosed herein, the acid material of choice may be aconcentrated acid with an average molarity (M) of at least 7 or above.In certain procedures, the average molarity will be at least 10 orabove; with an average molarity between 7 and 10 being useful in certainapplications. The acid material of choice employed may exist as a pureliquid, a liquid slurry or as an aqueous solution of the dissolved acidin essentially concentrated form.

Suitable acid materials can be either aqueous or non-aqueous materials.Non-limiting examples of suitable acid materials can include one or moreof the following: hydrochloric acid, nitric acid, phosphoric acid,chloric acid, perchloric acid, chromic acid, sulfuric acid, permanganicacid, prussic acid, bromic acid, hydrobromic acid, hydrofluoric acid,iodic acid, fluoboric acid, fluosilicic acid, fluotitanic acid.

In certain embodiments, the defined volume of a liquid concentratedstrong acid employed can be sulfuric acid having a specific gravitybetween 55° and 67° baume. This material can be placed in the reactionvessel and mechanically agitated at a temperature between 16° and 70° C.

In certain specific applications of the method disclosed, a measured,defined quantity of suitable hydroxide material can be added to anagitating acid, such as concentrated sulfuric acid, that is present inthe non-reactive vessel in a measured, defined amount. The amount ofhydroxide that is added will be that sufficient to produce a solidmaterial that is present in the composition as a precipitate and/or asuspended solid or colloidal suspension. The hydroxide material employedcan be a water-soluble or partially water-soluble inorganic hydroxide.Partially water-soluble hydroxides employed in the process as disclosedherein will generally be those which exhibit miscibility with the acidmaterial to which they are added. Non-limiting examples of suitablepartially water-soluble inorganic hydroxides will be those that exhibitat least 50% miscibility in the associated acid. The inorganic hydroxidecan be either anhydrous or hydrated.

Non-limiting examples of water-soluble inorganic hydroxides includewater soluble alkali metal hydroxides, alkaline earth metal hydroxidesand rare earth hydroxides; either alone or in combination with oneanother. Other hydroxides are also considered to be within the purviewof this disclosure. “Water-solubility” as the term is defined inconjunction with the hydroxide material that will be employed is defineda material exhibiting dissolution characteristics of 75% or greater inwater at standard temperature and pressure. The hydroxide that isutilized typically is a liquid material that can be introduced into theacid material. The hydroxide can be introduced as a true solution, asuspension or a super-saturated slurry. In certain embodiments, it iscontemplated that the concentration of the inorganic hydroxide inaqueous solution can be dependent on the concentration of the associatedacid to which it is introduced. Non-limiting examples of suitableconcentrations for the hydroxide material are hydroxide concentrationsgreater than 5 to 50% of a 5 mole material.

Suitable hydroxide materials include, but are not limited to, lithiumhydroxide, sodium hydroxide, potassium hydroxide, ammonium hydroxide,calcium hydroxide, strontium hydroxide, barium hydroxide, magnesiumhydroxide, and/or silver hydroxide. Inorganic hydroxide solutions whenemployed may have concentration of inorganic hydroxide between 5 and 50%of a 5 mole material, with concentration between 5 and 20% beingemployed in certain applications. The inorganic hydroxide material, incertain processes, can be calcium hydroxide in a suitable aqueoussolution such as is present as slaked lime.

In the process as disclosed, the inorganic hydroxide in liquid or fluidform is introduced into the agitating acid material in one or moremetered volumes over a defined interval to provide a defined resonancetime. The resonance time in the process as outlined is considered to bethe time interval necessary to promote and provide the environment inwhich the hydronium ion material as disclosed herein develops. Theresonance time interval as employed in the process as disclosed hereinis typically between 12 and 120 hours with resonance time intervalsbetween 24 and 72 hours and increments therein being utilized in certainapplications.

In various applications of the process, the inorganic hydroxide isintroduced into the acid at the upper surface of the agitating volume ina plurality of metered volumes. Typically, the total amount of inorganichydroxide material will be introduced as a plurality of measuredportions over the resonance time interval. Front-loaded metered additionbeing employed in many instances. “Front-loaded metered addition”, asthe term is used herein, is taken to mean addition of the totalhydroxide volume with a greater portion being added during the initialportion of the resonance time. An initial percentage of the desiredresonance time-considered to be between the first 25% and 50% of thetotal resonance time.

It is to be understood that the proportion of each metered volume thatis added can be equal or can vary based on such non-limiting factors asexternal process conditions, in situ process conditions, specificmaterial characteristics, and the like. It is contemplated that thenumber of metered volumes can be between 3 and 12. The interval betweenadditions of each metered volume can be between 5 and 60 minutes incertain applications of the process as disclosed. The actual additioninterval can be between 60 minutes to five hours in certainapplications.

In certain applications of the process, a 100 ml volume of 5% weight pervolume of calcium hydroxide material is added to 50 ml of 66° baumeconcentrated sulfuric acid in 5 metered increments of 2 ml per minute,with or without admixture. Addition of the hydroxide material to thesulfuric acid produces a material having increasing liquid turbidity.Increasing liquid turbidity is indicative of calcium sulfate solidsforming as precipitate. The produced calcium sulfate can be removed in afashion that is coordinated with continued hydroxide addition in orderto provide a coordinated concentration of suspended and dissolvedsolids.

Without being bound to any theory, it is believed that the addition ofcalcium hydroxide to sulfuric acid in the manner defined herein resultsin the consumption of the initial hydrogen proton or protons associatedwith the sulfuric acid resulting in hydrogen proton oxygenation suchthat the proton in question is not off-gassed as would be generallyexpected upon hydroxide addition. Instead, the proton or protons arerecombined with ionic water molecule components present in the liquidmaterial.

After the suitable resonance time as defined has passed, the resultingmaterial is subjected to a non-bi-polar magnetic field at a valuegreater than 2000 gauss; with magnetic fields great than 2 million gaussbeing employed in certain applications. It is contemplated that amagnetic field between 10,000 and 2 million gauss can be employed incertain situations. The magnetic field can be produced by varioussuitable means. One non-limiting example of a suitable magnetic fieldgenerator is found in U.S. Pat. No. 7,122,269 to Wurzburger, thespecification of which is incorporated by reference herein.

Solid material generated during the process and present as precipitateor suspended solids can be removed by any suitable means. Such removalmeans include, but need not be limited to, the following: gravimetric,forced filtration, centrifuge, reverse osmosis and the like.

The stable electrolyte composition of matter as disclosed herein is ashelf-stable viscous liquid that is believed to be stable for at leastone year when stored at ambient temperature and between 50 to 75%relative humidity. The stable electrolyte composition of matter can beuse neat in various end use applications. The stable electrolytecomposition of matter can have a 1.87 to 1.78 molar material thatcontains 8 to 9% of the total moles of acid protons that are not chargedbalanced.

The stable electrolyte composition of matter which results from theprocess as disclosed herein has molarity of 200 to 150 M strength, and187 to 178 M strength in certain instances, when measured titramtricallythough hydrogen coulometry and via FFTIR spectral analysis. The materialhas a gravimetric range greater than 1.15; with ranges greater than 1.9in in certain instances. The material, when analyzed, is shown to yieldup to 1300 volumetric times of orthohydrogen per cubic ml versushydrogen contained in a mole of water.

It is also contemplated that the composition of matter as disclosed canbe introduced into a suitable polar solvent and will result in asolution having concentration of hydronium ions greater than 15% byvolume. In some applications, the concentration of hydronium ions can begreater than 25% and it is contemplated that the concentration ofhydronium ions can be between 15 and 50% by volume.

The suitable polar solvent can be either aqueous, organic or a mixtureof aqueous and organic materials. In situations where the polar solventincludes organic components, it is contemplated that the organiccomponent can include at least one of the following: saturated and/orunsaturated short chain alcohols having less than 5 carbon atoms, and/orsaturated and unsaturated short chain carboxylic acids having less than5 carbon atoms. Where the solvent comprises water and organic solvents,it is contemplated that the water to solvent ratio will be between 1:1and 400:1, water to solvent, respectively. Non-limiting examples ofsuitable solvents include various materials classified as polar proticsolvents such as water, acetic acid, methanol, ethanol, n-propanol,isopropanol, n-butanol, formic acid and the like.

The ion complex that is present in the solvent material resulting fromthe addition of the composition of matter as defined therein isgenerally stable and capable of functioning as an oxygen donor in thepresence of the environment created to generate the same. The materialmay have any suitable structure and solvation that is generally stableand capable of functioning as an oxygen donor. Particular embodiments ofthe resulting solution will include a concentration of the ion asdepicted by the following formula:

$\lbrack {H_{x}O_{\frac{({x - 1})}{2}}} \rbrack +$

-   -   wherein x is an odd integer ≥3.

It is contemplated that ionic version of the compound as disclosedherein exists in unique ion complexes that have greater than sevenhydrogen atoms in each individual ion complex which are referred to inthis disclosure as hydronium ion complexes. As used herein, the term“hydronium ion complex” can be broadly defined as the cluster ofmolecules that surround the cation H_(x)O_(x-1)+ where x is an integergreater than or equal to 3. The hydronium ion complex may include atleast four additional hydrogen molecules and a stoichiometric proportionof oxygen molecules complexed thereto as water molecules. Thus, theformulaic representation of non-limiting examples of the hydronium ioncomplexes that can be employed in the process herein can be depicted bythe formula:

$\lbrack {{H_{x}O_{\frac{({x - 1})}{2}}} + ( {H_{2}O} )_{y}} \rbrack$

-   -   where x is an odd integer of 3 or greater; and    -   y is an integer from 1 to 20, with y being an integer between 3        and 9 in certain embodiments.

In various embodiments disclosed herein, it is contemplated that atleast a portion of the hydronium ion complexes will exist as solvatedstructures of hydronium ions having the formula:H_(S) +xO_(2y)+

-   -   wherein x is an integer between 1 and 4; and    -   y is an integer between 0 and 2.

In such structures, an

$\lbrack {H_{x}O_{\frac{({x - 1})}{2}}} \rbrack +$core is protonated by multiple H₂O molecules. It is contemplated thatthe hydronium complexes present in the composition of matter asdisclosed herein can exist as Eigen complex cations, Zundel complexcations or mixtures of the two. The Eigen solvation structure can havethe hydronium ion at the center of an H₉O₄+ structure with the hydroniumcomplex being strongly bonded to three neighboring water molecules. TheZundel solvation complex can be an H₅O₂+ complex in which the proton isshared equally by two water molecules. The solvation complexes typicallyexist in equilibrium between Eigen solvation structure and Zundelsolvation structure. Heretofore, the respective solvation structurecomplexes generally existed in an equilibrium state that favors theZundel solvation structure.

The present disclosure is based, at least in part, on the unexpecteddiscovery that stable materials can be produced in which hydronium ionexists in an equilibrium state that favors the Eigen complex. Thepresent disclosure is also predicated on the unexpected discovery thatincreases in the concentration of the Eigen complex in a process streamcan provide a class of novel enhanced oxygen-donor oxonium materials.

The process stream as disclosed herein can have an Eigen solvation stateto Zundel solvation state ratio between 1.2 to 1 and 15 to 1 in certainembodiments; with ratios between 1.2 to 1 and 5 to 1 in otherembodiments.

The novel enhanced oxygen-donor oxonium material as disclosed herein canbe generally described as a thermodynamically stable aqueous acidsolution that is buffered with an excess of proton ions. In certainembodiments, the excess of protons ions can be in an amount between 10%and 50% excess hydrogen ions as measured by free hydrogen content.

It is contemplated that oxonium complexes employed in the processdiscussed herein can include other materials employed by variousprocesses. Non-limiting examples of general processes to producehydrated hydronium ions are discussed in U.S. Pat. No. 5,830,838, thespecification of which is incorporated by reference herein.

The composition disclosed herein has the following chemical structure:

$\lbrack {H_{x}O_{\frac{({x - 1})}{2}}} \rbrack +$

-   -   wherein x is an odd integer ≥3;    -   y is an integer between 1 and 20; and    -   Z is a polyatomic or monatomic ion.

The polyatomic ion employed can be an ion derived from an acid havingthe ability to donate one or more protons. The associated acid can beone that would have a pKa values ≥1.7 at 23° C. The ion employed can beone having a charge of +2 or greater. Non-limiting examples of such ionsinclude sulfate, carbonate, phosphate, chromate, dichromate,pyrophosphate and mixtures thereof. In certain embodiments, it iscontemplated that the polyatomic ion can be derived from mixtures thatinclude polyatomic ion mixtures that include ions derived from acidshaving pKa values ≤1.7.

In certain embodiments, the composition of matter can have the followingchemical structure:

$\lbrack {{H_{x}O_{\frac{({x - 1})}{2}}} + ( {H_{2}O} )_{y}} \rbrack Z$

-   -   wherein x is an odd integer between 3-11;    -   y is an integer between 1 and 10; and    -   Z is a polyatomic ion or monoatomic ion.

The polyatomic ion can be derived from an ion derived from an acidhaving the ability to donate on or more protons. The associated acid canbe one that would have a pK_(a) values ≥1.7 at 23° C. The ion employedcan be one having a charge of +2 or greater. Non-limiting examples ofsuch ions include sulfate, carbonate, phosphate, oxalate, chromate,dichromate, pyrophosphate and mixtures thereof. In certain embodiments,it is contemplated that the polyatomic ion can be derived from mixturesthat include polyatomic ion mixtures that include ions derived fromacids having pK_(a) values ≤1.7.

In certain embodiments, the composition of matter is composed of astoichiometrically balanced chemical composition of at least one of thefollowing: hydrogen (1+), triaqua-μ3-oxotri sulfate (1:1); hydrogen(1+), triaqua-μ3-oxotri carbonate (1:1), hydrogen (1+),triaqua-μ3-oxotri phosphate, (1:1); hydrogen (1+), triaqua-μ3-oxotrioxalate (1:1); hydrogen (1+), triaqua-μ3-oxotri chromate (1:1) hydrogen(1+), triaqua-μ3-oxotri dichromate (1:1), hydrogen (1+),triaqua-μ3-oxotri pyrophosphate (1:1), and mixtures thereof in admixturewith a polar solvent selected from the group consisting of.

In order to better understand the invention disclosed herein, thefollowing examples are presented. The examples are to be consideredillustrative and are not to be viewed as limiting the scope of thepresent disclosure or claimed subject matter.

Example I

A novel composition of matter as disclosed herein is prepared by placing50 ml of concentrated liquid sulfuric acid having a mass fraction H₂SO₄of 98%, an average molarity (M) above 7 and a specific gravity of 66°baume in a non-reactive vessel and maintained at 25° C. with agitationby a magnetic stirrer to impart mechanical energy of 1 HP to the liquid.

Once agitation has commenced, a measured quantity of sodium hydroxide isadded to the upper surface of the agitating acid material. The sodiumhydroxide material employed is a 20% aqueous solution of 5M calciumhydroxide and is introduced in five metered volumes introduced at a rateof 2 ml per minute over an interval of five hours with to provide aresonance time of 24 hours. The introduction interval for each meteredvolume is 30 minutes.

Turbidity is produced with addition of calcium hydroxide to the sulfuricacid indicating formation of calcium sulfate solids. The solids arepermitted to precipitate periodically during the process and theprecipitate removed from contact with the reacting solution.

Upon completion of the 24-hour resonance time, the resulting material isexposed to a non-bi-polar magnetic field of 2400 gauss resulting in theproduction of observable precipitate and suspended solids for aninterval of 2 hours. The resulting material is centrifuged and forcefiltered to isolate the precipitate and suspended solids

Example II

The material produced in Example I is separated into individual samples.Some are stored in closed containers at standard temperature and 50%relative humidity to determine shelf-stability. Other samples aresubjected to analytical procedures to determine composition. The testsamples are subjected to FFTIR spectra analysis and titrated withhydrogen coulometry. The sample material has a molarity ranging from 187to 178 M strength. The material has a gravimetric range greater than1.15; with ranges greater than 1.9 in certain instances. The compositionis stable and has a 1.87 to 1.78 molar material that contains 8 to 9% ofthe total moles of acid protons that are not charged balanced. FFTIRanalysis indicates that the material has the formula hydrogen (1+),triaqua-μ3-oxotri sulfate (1:1).

Example III

A 5 ml portion of the material produced according to the method outlinedin Example I is admixed in a 5 ml portion of deionized and distilledwater at standard temperature and pressure. The excess hydrogen ionconcentration is measured as greater than 15% by volume and the pH ofthe material is determined to be 1.

While the invention has been described in connection with what ispresently considered to be the most practical and preferred embodiment,it is to be understood that the invention is not to be limited to thedisclosed embodiments but, on the contrary, is intended to cover variousmodifications and equivalent arrangements included within the spirit andscope of the appended claims, which scope is to be accorded the broadestinterpretation so as to encompass all such modifications and equivalentstructures as is permitted under the law

What is claimed is:
 1. A stoichiometrically balanced chemical compoundselected from the group consisting of at least one of the following:hydrogen (1+), triaqua-μ3-oxotri sulfate (1:1); hydrogen (1+),triaqua-μ3-oxotri carbonate (1:1), hydrogen (1+), triaqua-μ3-oxotriphosphate, (1:1); hydrogen (1+), triaqua-μ3-oxotri oxalate (1:1);hydrogen (1+), triaqua-μ3-oxotri chromate (1:1) hydrogen (1+),triaqua-μ3-oxotri dichromate (1:1), hydrogen (1+), triaqua-μ3-oxotripyrophosphate (1:1), and mixtures thereof.
 2. The stoichiometricallybalanced chemical compound of claim 1 wherein the stoichiometricallybalanced chemical compound is a stable electrolyte present in a polarsolvent, the polar solvent selected from the group consisting of water,short chain alcohols having between 1 and 4 carbon atoms and mixturesthereof an about between about 0.05% and 50% by volumes.
 3. Thestoichiometrically balanced chemical compound of claim 2 wherein atleast a portion of the chemical compound is present as H₉O₄+ incoordinated combination with H₉O₄+:SO₄H and working bridging ligandscontaining stable hydronium (H₃O+) clusters.
 4. The chemical compound ofclaim 3 wherein the stable electrolyte is present in an amountsufficient to provide an effective pKa of between 0 and
 5. 5. Thechemical compound of claim 3 wherein the stable electrolyte is presentin an amount sufficient to provide an effective hydronium ionconcentration between about 1 ppm and about 25% by volume.